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26 February, 02:06

Decomposition of N2O5 follows first order kinetics and its instantaneous rate is 1.6 x 10^-6 mol/L/s. Calculate the rate constant of the reaction of 0.02M solution.

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  1. 26 February, 02:51
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    8*10^-5 s^-1

    Explanation:

    The decomposition of N2O5 is shown by the reaction equation;

    N2O5 (aq) ⇄NO2 (g) + NO3 (g)

    We have the following information;

    Instantaneous rate of reaction = 1.6 x 10^-6 mol/L/s.

    Concentration of the N2O5 = 0.02M

    Now the rate of decomposition of N2O5 is given by;

    R = k[N2O5] (first order reaction)

    Hence;

    1.6 x 10^-6 mol/L/s = k[0.02M]

    k = 1.6 x 10^-6 mol/L/s / 0.02M

    k = 8*10^-5 s^-1

    Hence the rate of decomposition of N2O5 is 8*10^-5 s^-1
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